Question

he heat of fusion of tetrahydrofuran is . Calculate the change in entropy when of tetrahydrofuran melts at . Be sure your answer contains a unit symbol. Round your answer to significant digits.

Answer 1

`\Delta S=1.8x10^(-3)(kJ)/(K)=1.8(J)/(K)`

Step-by-step explanation:

Hello.

In this case, given the heat of fusion of THF to be 8.5 kJ/mol and freezing at -108.5 °C, for the required mass of 5.9 g, we can compute the entropy as:

`\Delta S=(n*\Delta H)/(T)`

Whereas n accounts for the moles which are computed below:

`n=5.9g*(1mol)/(72g) =0.082mol`

Thus, the entropy turns out:

`\Delta S=(0.0819mol*8.5 kJ/mol)/((-108.5+273.15)K)\\\\\Delta S=1.8x10^(-3)(kJ)/(K)=1.8(J)/(K)`

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